Problem: Calculate the percent ionization of a 0.15 M formic acid solution in a solution containing 0.11 M potassium formate.

FREE Expert Solution

We are asked to calculate the percent ionization of a 0.15 M formic acid solution in a solution containing 0.11 M potassium formate.


Recall that the percent ionization is given by:


% ionization=[H3O+][HA]initial×100


Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case). 



The dissociation of formic acid is as follows:

HCOOH(aq) + H2O(l) H3O+(aq) + HCOO(aq)


It has a Ka value of 1.8x10­-4 that can be found from a textbook or the internet.


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Problem Details

Calculate the percent ionization of a 0.15 M formic acid solution in a solution containing 0.11 M potassium formate.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.

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